Description

Checking Particles. Numbering Particles. There are basic units to tally things. Numbering Particles. There are regular units to number things. Pair. Numbering Particles. There are normal units to check things. Pair = 2Dozen . Numbering Particles. There are basic units to number things. Pair = 2Dozen = 12Ream.

Transcripts

The Mole Chap. 11 No, not that mole!

Counting Particles

Counting Particles There are basic units to check things

Counting Particles There are regular units to tally things Pair

Counting Particles There are normal units to tally things Pair = 2 Dozen

Counting Particles There are basic units to tally things Pair = 2 Dozen = 12 Ream

Counting Particles There are basic units to tally things Pair = 2 Dozen = 12 Ream = 500 sheets Gross

Counting Particles There are basic units to tally things Pair = 2 Dozen = 12 Ream = 500 Gross = 144 "Scop" (not by any means)

Counting Particles There are basic units to tally things Pair = 2 Dozen = 12 Ream = 500 Gross = 144 "Scop" (not by any means) = 64 Mole

Counting Particles There are basic units to tally things Pair = 2 Dozen = 12 Ream = 500 Gross = 144 "Scop" (not by any means) = 64 Mole = Avogadro\'s #

Avogadro\'s number An esteem equivalent to 6.0221367 x 10 23 . We\'ll round it to: 6.02 x 10 23

Counting Particles Converting with moles Finding the quantity of particles from moles.

Self Check – Ex. 1 what number particles are in 2 moles of helium?

Self Check – Ex. 2 what number particles are in 7.5 moles of carbon dioxide?

Counting Particles Converting with moles Finding the quantity of particles from moles. Finding the quantity of moles from particles.

Self Check – Ex. 3 A specimen of lead contains 1.5 x 10 24 iotas. What number of moles of lead particles are there?

Self Check – Ex. 4 An example of zinc chloride contains 2.150 x 10 18 equation units. What number of moles of zinc chloride are there?

Massing a Mole Different molecules have distinctive masses.

1 particle of carbon would weigh ____ times more than 1 iota of helium. 3

dozen iotas 1 particle of carbon would weigh ____ times more than 1 molecule of helium. 3 dozen particles

mole of 1 molecule of carbon would weigh ____ times more than 1 iota of helium. 3 mole of

Massing a Mole Different particles have distinctive masses. The mass on the P.T. speaks to. . .

Massing a Mole Different particles have distinctive masses. The mass on the P.T. speaks to. . . The mass of 1 particle (in amu)

Massing a Mole Different iotas have distinctive masses. The mass on the P.T. speaks to. . . The mass of 1 particle (in amu) The mass of 1 mole of molecules (in grams)

Massing a Mole Different iotas have diverse masses. The mass on the P.T. speaks to. . . This esteem is known as the molar mass. The mass of 1 mole of particles

If you weigh out 40 grams of argon you have basically checked ______________ iotas.

If you weigh out 40 grams of argon you have basically tallied ______________ iotas. 6.02 x 10 23

Massing a Mole Calculating with molar mass Using molar mass you can change over from to .

Massing a Mole Calculating with molar mass Using molar mass you can change over from grams to moles.

Self Check – Ex. 5 If an example of aluminum has a mass 81.0 g what number of moles are available?

Massing a Mole Calculating with molar mass Using molar mass you can change over from grams to moles. You can likewise change over from _____ to .

Massing a Mole Calculating with molar mass Using molar mass you can change over from grams to moles. You can likewise change over from moles to grams.

Self Check – Ex. 6 What is the mass of 0.25 moles of chromium?

Massing a Mole Calculating with molar mass Calculating the molar mass of compound

Example One mole of CH 4 contains: 1 mole of carbon moles of hydrogen

Example One mole of CH 4 contains: 1 mole of carbon 4 moles of hydrogen

Example One mole of CH 4 contains: 1 mole of carbon 4 moles of hydrogen measures 12 g weighs ______

Example One mole of CH 4 contains: 1 mole of carbon 4 moles of hydrogen measures 12 g measures 4 x (1) g

Example One mole of CH 4 contains: 1 mole of carbon 4 moles of hydrogen measures 12 g measures 4 x (1) g = 16 g/mol

Massing a Mole Calculating with molar mass Calculating the molar mass of compound Add the masses of each of the molecules in the compound.

Massing a Mole Calculating with molar mass Calculating the molar mass of compound Add the masses of each of the particles in the compound. Keep in mind to duplicate every iota\'s mass by the number iotas in the compound.

Self Check – Ex. 7 What is the molar mass of lithium nitrate, LiNO 3 ?

Self Check – Ex. 8 What is the molar mass of calcium acetic acid derivation, Ca(C 2 H 3 O 2 ) 2 ?

Molar Volume of Gas The volume of 1 mole of gas particles when measured at STP

Molar Volume of Gas This is resolved at particular conditions. STP – standard temperature (0 ºC) and standard weight (1 atm)

Molar Volume of Gas This is resolved at particular conditions. It\'s the same for all gasses. 1 mole of gas at STP = 22.4 L

Molar Volume of Gas This is resolved at particular conditions. It\'s the same for all gasses. Changes

Self Check – Ex. 9 What is the volume of 3 moles of carbon dioxide gas at STP?

Self Check – Ex. 10 what number moles of air are in a 64 L that is at 1 atm and 0 ºC.

Multiple progression transformations Just recall the mole is the focal unit

Mass (grams) Volume (liters) MOLE particles (iotas, atoms, recipe units)

Self Check – Ex. 11 What is the mass of 11.2 L of carbon dioxide gas?

Self Check – Ex. 12 what number atoms of alkali, NH 3 are in a 68-g test?

Mole proportions in concoction equations

Mole proportions in substance recipes The subscripts can give a proportion of iotas in a compound.

1 mole of smelling salts, NH 3 1 mole of N mole of N

1 mole of alkali, NH 3 1 mole of N 3 mole of N

1 mole of alkali, NH 3 1 mole of N 3 mole of N 1 mole NH 3 : 3 mole H 1 mole NH 3 : 1 mole N

1 mole of smelling salts, NH 3 1 mole of N 3 mole of N 1 mole NH 3 : 3 mole H 1 mole NH 3 : 1 mole N 1 mole NH 3 1 mole NH 3 1 mole N 1 mole N

Mole proportions in substance equations The subscripts can give a proportion of molecules in a compound. Changes

Self Check – Ex. 13 what number moles of hydroxide particles are in 1.2 moles of magnesium hydroxide, Mg(OH) 2 ?

Self Check – Ex. 14 What is the mass of the oxygen iotas in 4 moles of sodium sulfate?

The end.